logging in or signing up bonding in solids sudharani.kuram Download Post to : URL : Related Presentations : Share Add to Flag Embed Email Send to Blogs and Networks Add to Channel Uploaded from authorPOINT lite Insert YouTube videos in PowerPont slides with aS Desktop Copy embed code: (To copy code, click on the text box) Embed: URL: Thumbnail: WordPress Embed Customize Embed The presentation is successfully added In Your Favorites. Views: 721 Category: Education License: Some Rights Reserved Like it (2) Dislike it (0) Added: January 21, 2011 This Presentation is Public Favorites: 3 Presentation Description No description available. Comments Posting comment... By: chandusekhar (7 month(s) ago) plz let me download Saving..... Post Reply Close Saving..... Edit Comment Close By: chandusekhar (7 month(s) ago) plz let me download Saving..... Post Reply Close Saving..... Edit Comment Close By: chandusekhar (7 month(s) ago) please try to enable me to download Saving..... Post Reply Close Saving..... Edit Comment Close By: jamil2k2 (16 month(s) ago) Kindly let me download the presentation on Bonding in Solids. Regards J R Ansari Deep Inst. of Engg. & Tech. Saving..... Post Reply Close Saving..... Edit Comment Close Premium member Presentation Transcript Slide 1: TYPES OF BONDING IN SOLIDS Ionic bonding Covalent bonding Metallic bonding Hydrogen bonding Van der waals bonding Slide 2: IONIC BOND An ionic bonding is the attractive force existing between a positive ion and a negative ion when they are brought into close proximity. These ions are formed when the atoms of different elements involved lose or gain electrons in order to stabilise their outer shell electron configuration. Slide 3: Ionic bonding in sodium chloride Slide 4: STRUCTURE OF SODIUM CHLORIDE Slide 5: STRUCTURE OF SODIUM CHLORIDE Slide 6: STRUCTURE OF CESIUM CHLORIDE Slide 7: PROPERTIES OF IONIC SOLIDS Ionic solids are crystalline in nature They are hard and brittle. They have high melting and boiling points. Ionic solids are good insulators of electricity. Ionic solids are soluble in polar solvents and insoluble in non-polar solvents. In an ionic crystal, a cation is surrounded by as many as possible and vice-versa Slide 8: COVALENT BONDING In covalent bonding the stable arrangement of electrons in an outer shell is achieved by a process of valence electron sharing rather than electron transfer. Slide 9: A covalent bond may also be formed when two or more atoms of different non-metals share one or more pairs of valence electrons. Slide 10: COVALENT BOND IN CHLORINE Slide 11: COVALENT BONDING IN WATER MOLECULE Slide 12: COVALENT BONDING IN METHANE MOLECULE Slide 13: PROPERTIES OF COVALENT SOLIDS Covalent bonds are directional. They exhibit varying physical properties. Eg. Diamond is the hardest substance with high melting point.tin is very soft and has low melting point Covalent solids are hard and brittle. They possess crystalline nature. When compared with ionic solids, these solids have relatively low melting and boiling points. Pure covalent solids are good insulators of electricity at low temperatures. They are soluble in non polar solvents. Slide 14: Examples of ionic solids: NaCl KCl KBr MgO MgCl2 KOH Al2O3 Slide 15: When NaCl molecule is formed energy is released. This energy is called bond energy of the molecule which can be calculated from the formula V = - e2/4πЄoro Slide 16: EXAMPLES OF COVALENT SOLIDS sulphur Indium Germanium Silicon Graphite etc Slide 17: METALLIC BONDING The valence electrons from all the atoms belonging to the crystal are free to move throughout the crystal. The crystal may be considered as an array of positive metal ions embedded in a “cloud” or “sea” of free electrons. This type of bonding is called metallic bonding Slide 18: METALLIC BONDING Slide 19: METALLIC BONDING Slide 20: PROPERTIES OF METALLIC SOLIDS Metallic bonds hold the atoms together in metals. Metallic bonds are relatively weak. Metallic solids are malleable and ductile. Metallic bond is non directional. They have high number of free electrons. They possess high electrical and thermal conductivity. Metals are opaque to light. Metallic solids are not soluble in polar and non polar solvents. Metallic bonds are weaker than ionic polar and covalent bonds but stronger than van der waals bonds Slide 21: EXAMPLES OF METALLIC SOLIDS Sodium copper Gold silver Aluminium all metals Slide 22: HYDROGEN BONDING Covalently bonded atoms often produce an electric dipole configuration with hydrogen atom as the positive end of the dipole. If bonds arise as a result of electrostatic attraction between atoms, it is known as hydrogen bonding. Slide 23: HYDROGEN BONDING IN WATER MOLECULE Slide 24: HYDROGEN BOND IN WATER MOLECULES Slide 25: PROPERTIES OF HYDROGEN BONDED SOLIDS The hydrogen bonds are directional. The bonding is relatively strong as compared to other dipole-dipole interactions. Hydrogen bonded solids have low melting ponts. Since no valence electrons are available in such solids they are good insulators of electricity. They are soluble in both polar and non polar solvents. They are transparent to light. Since elements of low atomic numbers form such solids, they have low densities. Slide 26: EXAMPLES OF HYDROGEN BONDED SOLIDS water molecule in the form of ice ammonic molecules KH2PO4 Slide 27: The decrease in energy that takes place in the process of bringing the ions from an infinite distance to their equilibrium position in the stable lattice is called COHESIVE ENERGY. Slide 28: VAN DER WAALS BONDING Weak and temporary dipole bonds between molecules of the same substance are known as vander Waals bonding. You do not have the permission to view this presentation. In order to view it, please contact the author of the presentation.
bonding in solids sudharani.kuram Download Post to : URL : Related Presentations : Share Add to Flag Embed Email Send to Blogs and Networks Add to Channel Uploaded from authorPOINT lite Insert YouTube videos in PowerPont slides with aS Desktop Copy embed code: (To copy code, click on the text box) Embed: URL: Thumbnail: WordPress Embed Customize Embed The presentation is successfully added In Your Favorites. Views: 721 Category: Education License: Some Rights Reserved Like it (2) Dislike it (0) Added: January 21, 2011 This Presentation is Public Favorites: 3 Presentation Description No description available. Comments Posting comment... By: chandusekhar (7 month(s) ago) plz let me download Saving..... Post Reply Close Saving..... Edit Comment Close By: chandusekhar (7 month(s) ago) plz let me download Saving..... Post Reply Close Saving..... Edit Comment Close By: chandusekhar (7 month(s) ago) please try to enable me to download Saving..... Post Reply Close Saving..... Edit Comment Close By: jamil2k2 (16 month(s) ago) Kindly let me download the presentation on Bonding in Solids. Regards J R Ansari Deep Inst. of Engg. & Tech. Saving..... Post Reply Close Saving..... Edit Comment Close Premium member Presentation Transcript Slide 1: TYPES OF BONDING IN SOLIDS Ionic bonding Covalent bonding Metallic bonding Hydrogen bonding Van der waals bonding Slide 2: IONIC BOND An ionic bonding is the attractive force existing between a positive ion and a negative ion when they are brought into close proximity. These ions are formed when the atoms of different elements involved lose or gain electrons in order to stabilise their outer shell electron configuration. Slide 3: Ionic bonding in sodium chloride Slide 4: STRUCTURE OF SODIUM CHLORIDE Slide 5: STRUCTURE OF SODIUM CHLORIDE Slide 6: STRUCTURE OF CESIUM CHLORIDE Slide 7: PROPERTIES OF IONIC SOLIDS Ionic solids are crystalline in nature They are hard and brittle. They have high melting and boiling points. Ionic solids are good insulators of electricity. Ionic solids are soluble in polar solvents and insoluble in non-polar solvents. In an ionic crystal, a cation is surrounded by as many as possible and vice-versa Slide 8: COVALENT BONDING In covalent bonding the stable arrangement of electrons in an outer shell is achieved by a process of valence electron sharing rather than electron transfer. Slide 9: A covalent bond may also be formed when two or more atoms of different non-metals share one or more pairs of valence electrons. Slide 10: COVALENT BOND IN CHLORINE Slide 11: COVALENT BONDING IN WATER MOLECULE Slide 12: COVALENT BONDING IN METHANE MOLECULE Slide 13: PROPERTIES OF COVALENT SOLIDS Covalent bonds are directional. They exhibit varying physical properties. Eg. Diamond is the hardest substance with high melting point.tin is very soft and has low melting point Covalent solids are hard and brittle. They possess crystalline nature. When compared with ionic solids, these solids have relatively low melting and boiling points. Pure covalent solids are good insulators of electricity at low temperatures. They are soluble in non polar solvents. Slide 14: Examples of ionic solids: NaCl KCl KBr MgO MgCl2 KOH Al2O3 Slide 15: When NaCl molecule is formed energy is released. This energy is called bond energy of the molecule which can be calculated from the formula V = - e2/4πЄoro Slide 16: EXAMPLES OF COVALENT SOLIDS sulphur Indium Germanium Silicon Graphite etc Slide 17: METALLIC BONDING The valence electrons from all the atoms belonging to the crystal are free to move throughout the crystal. The crystal may be considered as an array of positive metal ions embedded in a “cloud” or “sea” of free electrons. This type of bonding is called metallic bonding Slide 18: METALLIC BONDING Slide 19: METALLIC BONDING Slide 20: PROPERTIES OF METALLIC SOLIDS Metallic bonds hold the atoms together in metals. Metallic bonds are relatively weak. Metallic solids are malleable and ductile. Metallic bond is non directional. They have high number of free electrons. They possess high electrical and thermal conductivity. Metals are opaque to light. Metallic solids are not soluble in polar and non polar solvents. Metallic bonds are weaker than ionic polar and covalent bonds but stronger than van der waals bonds Slide 21: EXAMPLES OF METALLIC SOLIDS Sodium copper Gold silver Aluminium all metals Slide 22: HYDROGEN BONDING Covalently bonded atoms often produce an electric dipole configuration with hydrogen atom as the positive end of the dipole. If bonds arise as a result of electrostatic attraction between atoms, it is known as hydrogen bonding. Slide 23: HYDROGEN BONDING IN WATER MOLECULE Slide 24: HYDROGEN BOND IN WATER MOLECULES Slide 25: PROPERTIES OF HYDROGEN BONDED SOLIDS The hydrogen bonds are directional. The bonding is relatively strong as compared to other dipole-dipole interactions. Hydrogen bonded solids have low melting ponts. Since no valence electrons are available in such solids they are good insulators of electricity. They are soluble in both polar and non polar solvents. They are transparent to light. Since elements of low atomic numbers form such solids, they have low densities. Slide 26: EXAMPLES OF HYDROGEN BONDED SOLIDS water molecule in the form of ice ammonic molecules KH2PO4 Slide 27: The decrease in energy that takes place in the process of bringing the ions from an infinite distance to their equilibrium position in the stable lattice is called COHESIVE ENERGY. Slide 28: VAN DER WAALS BONDING Weak and temporary dipole bonds between molecules of the same substance are known as vander Waals bonding.